Question

Is \[{\text{AgBr}}\] soluble in water?

Answer 1

Hint: We know that a solid, liquid, or gaseous chemical component (referred to as the solute)'s capacity to dissolve in a solvent (typically a liquid) and form a solution is known as solubility. A substance's solubility is mostly determined by the solvent employed, as well as temperature and pressure. The solubility of a substance in a particular solvent can be measured by the concentration of the saturated solution.

Complete answer:
We know that,
According to Solubility Rule,
Salts of:
- Group I elements (\[{\text{L}}{{\text{i}}^{\text{ + }}}\],\[{\text{N}}{{\text{a}}^ + }\], \[{{\text{K}}^ + }\], \[{\text{C}}{{\text{s}}^ + }\],\[{\text{R}}{{\text{b}}^ + }\])are soluble
- \[{\text{N}}{{\text{H}}_{{4^{}}}}^ + \] (Ammonium ion) are soluble
- The nitrate ions (\[{\text{N}}{{\text{O}}_3}^ - \]) are generally soluble.
- \[{\text{C}}{{\text{l}}^{\text{ - }}}\], \[{\text{B}}{{\text{r}}^{\text{ - }}}\],\[{{\text{I}}^{^{\text{ - }}}}\]are soluble. Exceptions: \[{\text{A}}{{\text{g}}^{\text{ + }}}\], \[{\text{P}}{{\text{b}}_{{{\text{2}}^{}}}}^{\text{ + }}\],\[{\left( {{\text{H}}{{\text{g}}_{\text{2}}}} \right)^2}^{\text{ + }}\]
- Most sulfates are soluble. Exceptions: \[{\text{B}}{{\text{a}}^{{\text{2 + }}}}\],\[{\text{C}}{{\text{a}}^{{\text{2 + }}}}^{}\],\[{\text{P}}{{\text{b}}^{{\text{2 + }}}}\],\[{\text{A}}{{\text{g}}^{{{\text{ + }}^{}}}}\],\[{\text{S}}{{\text{r}}^{{\text{2 + }}}}\]
- Most hydroxide salts are only slightly soluble. Exceptions: \[{\text{N}}{{\text{H}}_{\text{4}}}^{\text{ + }}\],\[{\text{L}}{{\text{i}}^{\text{ + }}}\] , \[{\text{N}}{{\text{a}}^{\text{ + }}}\],\[{{\text{K}}^ + }\]
- Most carbonates \[\left( {{\text{C}}{{\text{O}}_{\text{3}}}^{{\text{2 - }}}} \right)\] are insoluble. Exceptions: Group 1 and \[{\text{N}}{{\text{H}}_{\text{4}}}^{\text{ + }}\]
It should be kept in mind that rules at the top supersede any lower rules.
Thus, silver bromide is water insoluble and it also forms a pale yellow precipitate. A pale yellow hue solid is deposited at the bottom of the aqueous solution if it is explained in another way. It does not break down into its ions in water, despite being an ionic compound.

Note:
 It also has to do with the low electronegativity difference between silver and bromine, as well as a concept known as "Fajan's Rule," which states that silver's ionic radius is similar in size to halide ionic radii, allowing them to "snuggle up close," making them difficult to dissociate in water. It must be noted that at $200^\circ C$, \[{\text{AgBr}}\]has a solubility of $0.140mg/L$ in water. As a result, it has a very low value, proving that \[{\text{AgBr}}\]is a precipitate.